Video transcript
- [Instructor] In thisvideo, we're gonna look at the SN1 mechanism, and we'llstart with our alkyl halide. In the first step of our SN1 mechanism, we get loss of a leaving group, so the electrons in this bond come off onto the bromine to form the bromide ion. When that happens, we take a bond away from this carbon in red,so the carbon in red gets a plus one formal charge. Let me draw that in here. So the carbon in red is this one. It now has a plus one formal charge, and we have a carbocation. The carbon in red wentfrom being sp3 hybridized in our alkyl halide tobeing sp2 hybridized in our carbocation,which means the geometry directly around thecarbon in red is planar. We also have our bromine,so let me draw that in here. It has four lone pairs ofelectrons around it now, which gives it a negativeone formal charge. That's the bromide ion. The electrons in thisbond, these electrons in here come off onto the bromine to form our bromide ion,which is a good leaving group. In the first step of our SN1 mechanism, we get loss of a leaving group. And when that happens,we form our carbocation, and our carbocation has a plus one formal charge on this carbon. This is gonna functionas our electrophile. And our nucleophile will be the hydrosulfide ionwith a negative charge. Opposite charges attract,and in the second step of our mechanism, our nucleophileattacks our electrophile. On our second step weget nucleophilic attack, so nucleophilic attack, anda lone pair of electrons on our sulfur form a bondwith our carbon in red. In our final product, this is our carbon in red, and I'll highlight a lone pair of electrons on thissulfur, and that lone pair forms this bond to give us our product. Let's go to the video so we can see this mechanism using a model set. Here's our alkyl halide, and I'm saying that the green is our bromine. In the first step of our mechanism, we get loss of a leavinggroup, so these electrons come off onto our bromine to form the bromide ion, and weform our carbocation. But using this model set, it doesn't look like we have a planar carbocation. Those carbons are not in the same plane, so let me grab another model set here. You can see that,actually, those carbons are in the same plane, and we have an sp2 hybridized carbon in the center. If we look at thecarbocation from a top view, we can see the drawing, right? That's how we draw it in our mechanism. Next, our nucleophile comes along, which is our hydrosulfide ion, and our nucleophile could attack from either above or below, since we have a planar carbocation that is flat. Either way, we get the same product, so let's show the final product here. We're back to an sp3 hybridized carbon, so we have tetrahedralgeometry in our final product. The first step of our mechanism, loss of a leaving group,turns out to be the slow step, and the second step, nucleophilic attack, turns out to be the fast step. And this mechanism is consistentwith the experimentally determined rate law for this reaction. The rate of the reaction isequal to the rate constant, k, times the concentrationof our alkyl halide. So experiments have determined this to be our rate law, andthis is the concentration of our alkyl halide to the first power. The rate of the reaction depends on the concentration of the alkyl halide, but not on the concentrationof the nucleophile. And that's because ourfirst step is our slow step, and this is our rate determining step, if you remember this stufffrom general chemistry. And that means if youincrease the concentration of our alkyl halide, if youincrease the concentration of our alkyl halide by a factor of two, you increase the rate by a factor of two, since it's first order withrespect to our alkyl halides. But, if you try toincrease the concentration of your nucleophile, solet's say you increase the concentration of yournucleophile by a factor of two, there's no effect on the rate. This is zero order withrespect to our nucleophile. Our nucleophile can't attack until our carbocation is formed,and that's dependent only on the concentrationof our alkyl halide. So that's why this reaction is first order with respect to our alkyl halides. We call this an SN1 reaction, so the S stands for Substitution, the N stands for Nucleophilic, and the one refers to the fact that this is a unimolecular, this is a unimolecular reaction, which means that the rate of the reaction depends on the concentrationof only one thing, which is our substrate, our alkyl halide. So it's first order withrespect to our alkyl halide, and the nucleophilic substitution means that our nucleophile has substituted for our leaving group in our product. So that's an SN1 mechanism. The structure of the substrate also affects the rate of the reaction. If we start with a tertiary alkyl halide, like we did in the example above, we're gonna get a tertiary carbocation. So if these electronscome off onto the bromine, we're left with a tertiary carbocation, a plus one formal charge on this carbon. And we know that tertiarycarbocations are the most stable. We saw this in an earlier video. The more alkyl groups youhave, the more electron density you can donate to helpstabilize this positive charge. If we started with asecondary alkyl halide, when these electrons cameoff onto the bromine, we'd be left with a secondary carbocation. So let me draw this in here. And a secondary carbocationis only stabilized by two alkyl groups, so in this case, it'd be these two methyl groups here. And since a secondarycarbocation is not as stable as a tertiary, a tertiary carbocation would form a lot faster. So tertiary alkyl halides are the most reactive in an SN1 mechanism. A primary alkyl halide or a methyl halide, these wouldn't have avery stable carbocation, so the carbocation istoo unstable to exist, so generally, a primary alkyl halide does not react via an SN1 mechanism. And same with a methyl halide. In the previous example,we had a nucleophile with a negative one formal charge on it. What do you do if yournucleophile is neutral? In this case, the watermolecule has no charge on the oxygen, but it could still act as a nucleophile in our SN1 mechanism. Our first step is loss of a leaving group, so these electrons come off onto chlorine to form the chloride anion, and we're taking a bond away fromthis carbon in red. So that carbon in red is gonnaget a plus one formal charge. We draw our carbocation to try to show the planar geometry aroundthat central carbon here, which has a plus one formal charge. And then the next step, we know our nucleophile attacks our electrophile. So our nucleophile has this oxygen with a partial negative charge, right? The oxygen's more electronegativethan these hydrogens, so it withdraws some electron density. And a lone pair of electrons here on this oxygen can forma bond with this carbon. So our nucleophileattacks our electrophile, and let's draw what we would form. Let me draw in these groups here, and then we'd have our oxygen, which is now bonded to our carbon, and our oxygen is stillbonded to two hydrogens. Let me show the electrons in magenta here, forming a bond between thisoxygen and our carbons. So the electrons in magentawould be these electrons. We still have a lone pair of electrons on the oxygen that's leftover, so that's this lone pair. Let me draw those in, and that would give this oxygen a plus one formal charge. If we compare this with our final product, notice we only need to doa proton transfer, right? An acid-base reaction. Another molecule of water could come along and act as a base. Let me draw that in here. And it could take one of these protons, so it could take this, andleave these electrons behind on the oxygen, so let'shighlight those electrons in red. So these electrons in red here end up on that oxygen, and ourfinal product is neutral. We have no charge, andwe form tert-Butanol. This is called a solvolysis reaction. Let me write that in here. This is a solvolysis reaction, which just means that oursolvent is the nucleophile. Our solvent is water, which also functions as the nucleophile in this mechanism.
